A student electrolyzes an aqueous solution of \(\text{CuSO}_4\text{(aq)}\) to deposit copper metal onto a cathode. To deposit \(0.635 \text{ g}\) of \(\text{Cu(s)}\) in \(965 \text{ s}\), what constant electrical current, in amperes, must be passed through the cell? (Faraday's constant = \(96,500 \text{ C/mol } e^-\); molar mass of \(\text{Cu} = 63.5 \text{ g/mol}\))